ORIGINAL PAPER
Close contacts involving germanium and tin in crystal structures:
experimental evidence of tetrel bonds
Patrick Scilabra
1&Vijith Kumar
1&Maurizio Ursini
1&Giuseppe Resnati
1Received: 9 November 2017 / Accepted: 14 December 2017 / Published online: 8 January 2018 # The Author(s) 2018. This article is an open access publication
Abstract
Modeling indicates the presence of a region of low electronic density (a
Bσ-hole^) on group 14 elements, and this offers an
explanation for the ability of these elements to act as electrophilic sites and to form attractive interactions with nucleophiles.
While many papers have described theoretical investigations of interactions involving carbon and silicon, such investigations of
the heavier group 14 elements are relatively scarce. The purpose of this review is to rectify, to some extent, the current lack of
experimental data on interactions formed by germanium and tin with nucleophiles. A survey of crystal structures in the
Cambridge Structural Database is reported. This survey reveals that close contacts between Ge or Sn and lone-pair-possessing
atoms are quite common, they can be either intra- or intermolecular contacts, and they are usually oriented along the extension of
the covalent bond formed by the tetrel with the most electron-withdrawing substituent. Several examples are discussed in which
germanium and tin atoms bear four carbon residues or in which halogen, oxygen, sulfur, or nitrogen substituents replace one, two,
or three of those carbon residues. These close contacts are assumed to be the result of attractive interactions between the involved
atoms and afford experimental evidence of the ability of germanium and tin to act as electrophilic sites, namely tetrel bond (TB)
donors. This ability can govern the conformations and the packing of organic derivatives in the solid state. TBs can therefore be
considered a promising and robust tool for crystal engineering.
Keywords Tetrel bond . Crystal engineering .
σ-Hole interactions . Supramolecular interactions
Introduction
A comprehensive knowledge of the various interactions (i.e.,
weak bonds) that a molecule can participate in is a
fundamen-tal prerequisite for controlling and designing the conformation
and the packing that the molecule adopts in a crystal.
Interatomic distances that are slightly less than the sum of
the van der Waals radii of the atoms involved (hereafter
termed
Bclose contacts^) are usually (but not always) the
re-sult of attractive interactions between the involved atoms.
Observing the systematic occurrence of close contacts in
crys-talline solids can thus provide great insights into the attractive
interactions that atoms and molecular moieties can participate
in. Close contacts play a crucial role in the properties of
mat-ter, especially condensed phases, and knowledge and control
of these contacts enables the functional properties of
mate-rials—synthetic and natural—to be designed and optimized
[
1
–
3
].
Hydrogen bonds (HBs) are by far the most frequently
oc-curring and widely studied type of interaction [
4
,
5
]; other
weak interactions that have traditionally received attention
include
π–π [
6
], cation–π [
7
], anion–π [
8
], and aurophilic
[
9
] bonds.
σ-Hole interactions [
10
–
12
] represent a relatively
recent entry into the canon of weak bonds [
13
–
15
], but
fol-lowing the seminal papers of P. Politzer et al. [
16
,
17
], these
interactions rapidly became popular targets for studies in this
field [
15
,
18
–
20
]. A covalently bonded atom characteristically
has a region of low electron density, known as the
Bσ-hole,^
which is usually located along the extension of the covalent
bond but on the opposite side of the atom to the bond. The
electrostatic potential in this region is frequently positive and
σ-hole bonding is the result of an attractive interaction
be-tween this positive region (an electrophilic site, the donor site
in the interaction) and a negative site (a nucleophilic site, the
This paper belongs to Topical Collection P. Politzer 80th Birthday Festschrift
* Giuseppe Resnati giuseppe.resnati@polimi.it
1 NFMLab—D.C.M.I.C. BGiulio Natta^, Politecnico di Milano, Via L.
localized nature of the region(s) of positive electrostatic
po-tential. In an R–A···B interaction, where A is the atom with the
positive
σ-hole potential and B is the nucleophile, the angle
R–A···B is generally between 155° and 180°.
Experimental evidence and theoretical calculations
consis-tently show that most of the elements in groups 14–18 of the
periodic table form
σ-hole bonds. A growing consensus is
emerging among chemists that these interactions should be
named according to the group of the periodic table that the
electrophilic atom belongs to [
22
,
23
]. Halogen bonds (XBs)
[
10
,
24
], namely interactions where an atom of a group 17
element is the electrophilic site, represent the best known
sub-set of
σ-hole interactions. Chalcogen bonds (CBs) have been
studied in silico [
25
,
26
] and in the solid [
27
], liquid [
28
], and
gas [
29
] phases. Pnictogen bonds (PBs) have received much
attention in studies performed in silico [
30
] and in the solid
[
31
]; and the aerogen bond (AB) is the most recently
discov-ered subset of
σ-hole interactions [
32
].
The tetrel bond (TB), namely an interaction in which a
group 14 element is the electrophile, has received a great deal
of attention, probably due to the scale of its influence in
chem-istry, e.g., its possible role in SN2 reactions and hydrophobic
interactions [
13
,
33
]. The first convincing evidence of the
ability of carbon to attractively interact with
lone-pair-possessing atoms was reported more than forty years ago. In
1975, Johnson et al. calculated that the arrangement of the
water–carbon dioxide dimer in which there is close C···O
function as electrophiles describe theoretical investigations of
interactions involving carbon [
38
] and silicon [
39
–
41
],
where-as investigations of the heavier group 14 elements are far less
frequent [
42
]. Experimental studies of TBs are quite limited
[
29
,
43
–
45
] and, to the best of our knowledge, they have never
focused on interactions involving germanium or tin. We
there-fore decided to analyze structures in the Cambridge Structural
Database (CSD) in order to assess whether organic derivatives
of these two elements in crystalline solids show the presence
of TBs. We looked for systems in which germanium and tin
form close contacts with nucleophilic sites. Since
directional-ity is a key characteristic of
σ-hole interactions, particular
attention was paid in this survey to the geometrical features
of the observed close contacts, and a linear close contact was
considered to be a TB.
In this paper, we discuss a selected number of crystalline
structures of organic derivatives of germanium and tin in
which these elements form TBs, i.e., close linear contacts with
lone-pair-possessing heteroatoms. Structurally simple and
poorly functionalized molecular systems are preferentially
an-alyzed, as the Ge/Sn···nucleophile interactions that occur in
these systems are more likely to be a straightforward product
of the features of the two sites involved (contributions from
other parts of the molecule(s) are likely to be insignificant).
Wider coverage of organic Ge and Sn derivatives that present
TBs in the solid is given in the works cited in this review. The
interaction distances are analyzed based on the normalized
Fig. 1 Ball and stick representations (Mercury 3.9) of bis(methoxymethyl)phenyl)triphenyltin (MUBVOU, left) and (2,6-bis(ethoxymethyl)phenyl)dichlorophenyltin (LIVHOO, right). TBs are
depicted as black dotted lines; hydrogens have been omitted for clarity. Nc values are shown close to the respective interactions. Color code: gray carbon, green chlorine, red oxygen, dark teal tin
contact (Nc), defined as the ratio between the experimentally
observed separation of the interacting atoms and the sum of
their respective van der Waals radii [
46
].
1The use of Nc
values allows linear comparisons between contacts involving
different atoms. While the number of CSD structures in which
Ge/Sn···nucleophile interactions are present is not large
enough to enable definitive and detailed generalizations to
be made, the CSD survey reported here shows that the
forma-tion of attractive interacforma-tions between organic Ge and Sn sites
and a donor of electron density can become a determinant of
structure in crystalline solids. Intra- and intermolecular TBs
are observed, and they can affect the preferred conformation
of a molecule and/or the network of intermolecular
interac-tions in the crystal packing. Importantly, the cases collected
here provide convincing experimental evidence that TBs tend
to be more linear than PBs [
31
].
Oxygen atoms as TB acceptors
The conformation adopted by (2,6-bis(methoxymethyl)
phenyl)triphenyltin (refcode MUBVOU) in the crystal
(Fig.
1
, left) seems to be determined by two intramolecular
Sn···O TBs [
48
]. One interaction distance is slightly shorter
than the other, with the two Nc values being 0.76 and 0.78.
Shorter
σ-hole interactions usually tend to be more linear;
consistent with this characteristic, the two C–Sn···O angles
in the TBs mentioned above are 168.05° and 172.55°,
respec-tively. As discussed above, another common feature of
σ-hole
interactions is that the more electron-withdrawing the residue
covalently bonded to the
σ-hole donor site, the more positive
the
σ-hole, and the closer and stronger the interactions with
incoming nucleophiles. Interestingly, in an analog of the
com-pound discussed above wherein two of the phenyl rings are
replaced with chlorine atoms, the two intramolecular TBs
a r e
m u c h
s h o r t e r ;
i . e . ,
i n
( 2 , 6
-bis(ethoxymethyl)phenyl)dichlorophenyltin (refcode
1A van der Waals radius of 210 pm was adopted for germanium, as suggested
by Batsanov in [47].
Fig. 2 Ball and stick
representations (Mercury 3.9) of
methyl-tris((2-methoxymethyl)phenyl)germane (IMUTEP, top left), bromo-
tris((2-methoxymethyl)phenyl)germane (IMUTAL, top right), chloro-
tris((2-methoxymethyl)phenyl)germane (IMUSUE, bottom left), and
fluoro-tris((2-methoxymethyl)phenyl)germane (IMUSOY, bottom right). TBs are depicted as black dotted lines; hydrogens have been omitted for clarity. Nc values are shown close to the respective interactions. Color code: gray carbon, brown bromine, green chlorine, yellowish green fluorine, red oxygen, light teal germanium
LIVHOO), the Nc values for the Sn···O TBs are 0.66 and 0.78
(Fig.
1
, right) [
49
].
It is extensively documented that the propensity of a
halo-gen atom to form XBs increases with its molecular weight
[
10
], and that the heavier halogens usually form stronger and
shorter XBs than the lighter ones, with both of these behaviors
being independent of the XB acceptor. Similar trends are
ob-served when elements of groups 16 and 15 form CBs and PBs,
respectively. In all cases, this is probably due to the fact that
within a group of the periodic table, the polarizability
in-creases with the molecular weight of the element, and high
polarizability favors an anisotropic distribution of the electron
density around the atom and thus the strength of
σ-hole
inter-actions. It is no surprise [
50
] that
methyl-tris((2-methoxymethyl)phenyl)germane (refcode IMUTEP) shows
only one C–Ge···O contact, and that the corresponding Nc
value (0.87) is greater than the Nc values of the structurally
similar tin derivatives MUBVOU and LIVHOO [
51
] (Fig.
2
,
top left).
Bromine is more electronegative than carbon, and the Br–
Ge···O TB in bromo-tris((2-methoxymethyl)phenyl)germane
(refcode IMUTAL) is shorter (Nc = 0.79) than the C–Ge···O in
IMUTEP (Fig.
2
, top right) [
51
]; chlorine is more
electroneg-ative than bromine, and the Cl–Ge···O TB in
chloro-tris((2-methoxymethyl)phenyl)germane (refcode IMUSUE) is even
shorter (Nc = 0.76) (Fig.
2
, bottom left) than the Br–Ge···O
TB. Also, in these three structures, the linearity of the TB is
correlated with its length (the C–Ge···O, Br–Ge···O, and Cl–
Ge···O angles are 171.79°, 172.64°, and 173.24°,
respective-ly). In fluoro-tris((2-methoxymethyl)phenyl)germane
(refcode IMUSOY), a fluorine is substituted for the methyl
of IMUTEP and the depletion of electron density at
germani-um becomes large enough that two TBs are present (Fig.
2
,
bottom right). Consistent with the relative electronegativities
of fluorine and carbon, the F–Ge···O interaction is closer and
more directional than the C
–Ge···O interaction (the Nc values
for the Ge···O separations are 0.78 and 0.95, respectively).
Also, the presence of a tin-bonded iodine atom can promote
the formation of close contacts (Fig.
3
). Two independent
molecules are present in the unit cell of crystalline
iodo(2,6-bis(methoxymethyl)phenyl)diphenyltin (refcode RAKBOV),
Fig. 3 Ball and stick representation (Mercury 3.9) of the two molecules of the unit cell of iodo(2,6-bis(methoxymethyl)phenyl)diphenyltin (RAKBOV). TBs are depicted as black dotted lines; hydrogen atoms have been omitted for clarity. Nc values are shown close to the respective interactions. Color code: gray carbon, red oxygen, purple iodine, dark teal tin
Fig. 4 Ball and stick representations (Mercury 3.9) of one of the two independent molecules in the unit cells of (Z)-2-methyl-4-phenyl-3-(trimethylgermanyl)but-2-enoic acid (QIBDOV, left), (2-carbomethoxy-1,4-cyclohexadien-1-yl)trimethyltin (KASYOS, middle), and trans-N-t-butyloxycarbonyl-2-methyl-6-(trimethylstannyl)-4-phenyl)piperidine
(EABFES, right) derivatives. TBs are depicted as black dotted lines; hydrogen atoms have been omitted for clarity. Nc values are shown close to the respective interactions. Color code: gray carbon, red oxygen, light blue nitrogen, light teal germanium, dark teal tin Fig. 5 Ball and stick representations (Mercury 3.9) of 1D chains generated by ethyl trimethyltin diazoacetate (SIWRAR, top) and 2,5-bis(trimethylgermyl)thiophene-1,1-dioxide (QAHXIG, bottom). TBs are depicted as black dotted lines; hydrogen atoms have been omitted for clarity. Nc values are shown close to the respective interactions. Color code: gray carbon, red oxygen, light blue nitrogen, yellow sulfur, light teal germanium, dark teal tin
and in both of them the conformation is locked in by two
intramolecular TBs: an I–Sn···O and a C–Sn···O TB. The
dis-tances of the former interactions are shorter and those
interac-tions are more directional than the latter ones (the Nc values
are 0.70 and 0.72 for I–Sn···O and 0.79 and 0.81 for C–Sn···O;
the mean I
–Sn···O angle is 166.19° and the mean C–Sn···O
angle is 166.68°).
Carbonyl oxygen atoms can act as effective TB acceptors.
In (Z)-2-methyl-4-phenyl-3-(trimethylgermanyl)but-2-enoic
acid (refcode QIBDOV) [
52
], a short C–Ge···O contact is
present in both conformations adopted by the compound in
the crystals (Fig.
4
, left) (Nc for Ge···O is 0.80; the C
–Ge···O
angles are 174.17° and 175.00°), and a shorter TB occurs in a
trimethylstannylcarbomethoxy derivative (refcode KASYOS)
[
53
], where a similar tin-based tecton is present (Nc for C
–
Sn···O is 0.76) (Fig.
4
, middle). Similar TBs are given by the
carbonyl oxygens of carbamates (e.g.,
N-t-butyloxycarbonyl-2-methyl-6-trimethylstannyl-4-phenyl-piperidine, refcode
Fig. 6 Ball and stick representations (Mercury 3.9) of the 1D networks formed by N-triethylstannylsuccinimide (FUSZIC) due to N–Sn···O TBs (top), by N-chlorosuccinimide (CSUCIM) due to N–Cl···O XBs (middle), and by N-bromosuccinimide (NBSUCA) due to N–Br···O XBs (bottom). T h e t h r e e m e t h y l g r o u p s o f t h e e t h y l r e s i d u e s o f N -triethylstannylsuccinimide and hydrogen atoms have been deleted for the sake of simplicity. TBs and XBs are depicted as black dotted lines and green dotted lines, respectively. Color code: gray carbon, red oxygen, purple iodine, brown bromine, dark teal tin
Fig. 7 Ball and stick representation (Mercury 3.9) of the 1D network in which the ketone oxygen of O-tricyclohexyltin-4-oxo-4-phenylbutanoate (APAZIB) functions as the TB acceptor site. Hydrogen atoms and five of the cyclohexyl carbons have been deleted for the sake of simplicity. Color code: gray carbon, red oxygen, dark teal tin
Fig. 8 Ball and stick representation (Mercury 3.9) of the two-dimensional network formed by bis(tricyclohexyltin)nonanoate (CUXSOF). Five atoms of the cyclohexyl residues bound to tin have been deleted for the sake of simplicity. Color code: gray carbon, red oxygen, dark teal tin
EABFES; Nc = 0.75 and the C–Sn···O angle is 165.31°; Fig.
4
, right) [
54
,
55
] and several other carbonyl derivatives, e.g.,
amides [
56
], aldehydes [
57
,
58
], and ketones [
59
].
The CSD contains both intra- and intermolecular TBs that
have a carbonyl oxygen acting as the TB acceptor and
facili-tate the generation of discrete adducts [
60
] or infinite chains
(one-dimensional networks, 1D nets). In ethyl trimethyltin
diazoacetate (refcode SIWRAR) [
61
], the diazoacetate residue is
expected to form a
hole on tin that is more positive than the
σ-holes formed by the methyl groups. Consistent with this expectation,
a tetrel-bonded infinite chain is present in the crystal of the
com-pound (Fig.
5
, top), wherein the carbonyl oxygen approaches the tin
atom along the extension of the N2C–Sn covalent bond (the Sn···O
separation is 312.5 pm, which corresponds to an Nc value of 0.85;
the C–Sn···O angle is 176.46°). Similarly, the most positive σ-hole
on germanium in 2,5-bis(trimethylgermyl)thiophene-1,1-dioxide
(refcode QAHXIG) [
62
] is expected to occur opposite to the
O2
SC–Ge covalent bond, and an infinite chain (Fig.
5
, bottom) is
formed in which the sulfonyl oxygens approach germanium atoms
along the extension of each O2
SC–Ge covalent bond, leading to a
particularly linear geometry (the Ge···O separation corresponds to an
Nc value of 0.97, and the C
–Ge···O angle is 179.77°).
N-triethylstannylsuccinimide (refcode FUSZIC) [
63
] is a
self-complementary module that forms tetrel-bonded infinite
chains (one-dimensional networks, 1D nets) (Fig.
6
, top).
Consistent with the expected involvement of an sp
2lone pair
of the carbonyl oxygen as the nucleophilic site that interacts
with Sn along the extension of the N–Sn covalent bond, the
Sn···O=C angle is 138.28° and the tin atom is approximately
in the plane of the succinimide (the distance between the mean
square plane through the seven heavy atoms of the
succinimide moiety and the tetrel-bonded tin atom is
219 pm). The halogen-bonded infinite chains formed by
N-chloro- and N-bromosuccinimide (refcodes CSUCIM01 and
NBSUCA, respectively) [
64
] are also reported in Fig.
6
(mid-dle and bottom) in order to highlight the analogous
supramo-lecular features of TB and XB.
In several structures in the CSD, the tin atom of a
trialkylalkanoyltin moiety found in R3Sn–OC(O)R′
deriva-tives shows the presence of a TB with a carbonyl oxygen
located opposite to the covalent Sn–O bond, and
one-dimensional [
65
], two-dimensional [
66
], or
three-dimensional [
67
] networks are formed depending on the
over-all structure of the compound (Figs.
7
,
8
, and
9
).
Various other oxygen functionalities can act as donors of
electron density to organotin and germanium derivatives, e.g.,
water [
68
–
70
], sulfoxides and sulfones [
71
–
74
], as well as
Fig. 9 Ball and stick representation (Mercury 3.9) of the three-dimensional network with adamantanoid topology formed by bis(tri-n-butyltin)-1,2,2-trimethylcyclopentane-1,3-dicarboxylate (DIYFIB). Three atoms of the butyl residues bound to tin and the methyl pendants on the cyclopentyl rings have been deleted for the sake of simplicity. Color code: gray carbon, red oxygen, dark teal tin
Fig. 10 Ball and stick representations (Mercury 3.9) of the trimer formed by 1,3-bis(bromodimethylstannyl)propane and water (XINROB, top left), of the dimer formed by bro mo-tris( p-ethylphenyl)tin and hexamethylphosphoramide (HEVQIJ, top right), of the dimer formed by chlorotrimethyltin and triphenylphosphine oxide (HIGRUK01, bottom left), and of the dimer formed by chlorotriphenyltin and dimethyl sulfoxide (RUGYOI, bottom right). Hydrogen atoms and the 2,2′-bipyridine in XINROB have been deleted for the sake of simplicity. TBs are depicted as black dotted lines. Color code: gray carbon, red oxygen, blue nitrogen, orange phosphorus, green chlorine, brown bromine, yellow sulfur, dark teal tin
phosphine oxides, hexamethylphosphortriamide, and their
an-alogs [
75
–
81
] (Fig.
10
).
Nitrogen atoms as TB acceptors
The CSD contains several structures in which the nitrogen
atom of amine, pyridine, and cyano moieties forms a close
contact with a tin or germanium atom (Fig.
11
), thus showing
that—similar to oxygen atoms—nitrogen atoms can act as TB
acceptors, and this can be the case whether there is sp
3, sp
2, or
sp hybridization.
The ability of nitrogen atoms of tertiary amines to form
close contacts with organogermanium and -tin derivatives is
particularly well documented. For instance, two
symmetrical-ly nonequivalent molecules are present in crystals of
tris(2-((dimethylamino)methyl)phenyl)germane (refcode
GAGYIW) [
82
], and the conformations of both molecules
are influenced by three intramolecular C–Ge···N TBs
(Fig.
12
, left) (the Nc values of these TBs span the range
0.82–0.84, and the C–Ge···N angles vary between 172.45°
and 176.79°). The C–N–C angles vary between 109.70° and
113.25°, indicating that nitrogen atoms of the tertiary amine
moieties adopt a tetrahedral conformation and the lone pairs
align with the extensions of the covalent C
–Ge bonds, as
expected for
σ-hole interactions (the C–N···Ge angles span
the range 82.34–120.39°).
Imine nitrogen atoms behave in a similar manner to amine
nitro-gens. A close linear C–Ge···N interaction affects the conformation
adopted by
1-(trimethylsilylimino(diphenyl)phosphoranyl)-2-(triphenylgermyl)benzene (Nc for Ge···N is 0.85; the C
–Ge···N
angle is 173.79°) (refcode VIQXIC) [
83
] (Fig.
12
, right). In the
crystal of this compound, the P=N···Ge angle is 96.80°, and the
germanium atom is approximately in the iminophosphoranyl plane
(the distance between the tetrel-bonded germanium atom and the
mean square plane through the phosphorus, nitrogen, and silicon
atoms is 263 pm), suggesting that the lone pair at nitrogen aligns
with the extension of the covalent C–Ge bond.
Close intramolecular Ge···N contacts affect the conformation of a
family of 4,6,11-trioxa-1-aza-5-germabicyclo[3.3.3]undecanes
(germatrane derivatives). In the solid, 5-(t-butyl)-germatrane
(refcode BUWBUQ) [
84
] adopts an endo conformation (Fig.
13
,
left) where the C
–Ge···N separation is as short as 223.6 pm (Nc =
0.61). 5-Bromogermatrane (refcode BUWCUR) [
85
] behaves
sim-ilarly (Fig.
13
, middle), and the Br–Ge···N separation is even shorter
Fig. 11 Ball and stick representations (Mercury 3.9) of the dimer formed by chloro(trimethyl)tin and pyridine (CMEPSN, top left), of the trimer formed by chloro(tribenzyl)tin and 4,4′-bipyridyl (FEJFUW, top right), and of the 1D chain formed by chlorotris(4-cyanobenzyl)tin (BIBQIN, bottom). Hydrogen atoms have been deleted for the sake of simplicity. TBs are depicted as black dotted lines. Color code: gray carbon, blue nitrogen, green chlorine, dark teal tin
Fig. 12 Ball and stick representations (Mercury 3.9) of tris(2-((dimethylamino)methyl)phenyl)germane (GAGYIW, left) and 1( t r i m e t h y l s i l y l i m i n o 1( d i p h e n y l ) p h o s p h o r a n y l ) 2 -(triphenylgermyl)benzene (VIQXIC, right) derivatives. TBs are depicted
as black dotted lines; hydrogen atoms have been omitted for clarity. Nc values are shown close to the respective interactions. Color code: gray carbon, light blue nitrogen, yellow sulfur, pearl white silicon, orange phosphorus, light teal germanium
(208.4 pm, Nc = 0.57) than in BUWBUQ, consistent with the fact
that bromine is more electronegative than carbon and the
σ-hole
opposite the Br–Ge covalent bond is probably more positive than
that opposite the C–Ge bond. Analogous endo conformations and
Ge···N distances that are much shorter than the sum of the van der
Waals radii of the germanium and nitrogen atoms are observed in
other germatrane derivatives [
86
–
88
] and related systems [
89
,
90
]
(Fig.
13
, right). Similar behavior is encountered in the crystals of tin
analogs. 5-Methyl-1-aza-5-stannabicyclo[3.3.3]undecane (refcode
FEWXOU) [
79
] and its 5-fluoro [
91
], 5-chloro [
92
], 5-bromo
[
91
], and 5-iodo [
91
] analogs (refcodes ZANKEE, DAYMUL,
ZANKOO, ZANKUU, respectively) all show close Sn···N contacts
(Fig.
14
).
As in organogermanium derivatives, the nitrogen atom of the
2-(dimethylaminomethyl)phenylstannyl moiety forms an
intramo-lecular TB which affects the conformation of the respective
com-pound in the solid. This is the case for
(cyclopenta-2,4-dien-1-yl)-(2-(dimethylaminomethyl)phenyl)diphenyl tin (refcode
IHOZAH) [
93
] (Fig.
15
, left), where the intramolecular C–Sn···N
distance corresponds to an Nc value of 0.74 and the C–Sn···N angle
is 171.08°, congruent with an attractive interaction between the lone
pair of the tertiary amine nitrogen and the
σ-hole along the extension
of the C
–Sn covalent bond. Analogous Sn···N interactions are
pres-ent in structurally related derivatives [
94
–
96
]. A five-membered and
tetrel-bonded ring similar to that of IHOZAH is afforded by
(3-aminopropyl)triphenyltin (refcode COKVUV) [
97
] (Fig.
15
, right),
which shows an Sn···N interaction where Nc is 0.74 and the C–Sn···
N angle is 175.81°.
The tin atom of R3Sn
–OC(O)R′ derivatives is a good TB
donor and frequently interacts with the oxygen atom of a
carbonyl group (Figs.
7
–
9
) or the nitrogen atom of a pyridine
moiety. The intermolecular Sn···N interaction occurs opposite
to the covalent Sn–O bond, and discrete trimers [
98
] (Fig.
16
,
top) or one-dimensional [
99
–
102
] (Fig.
16
, bottom) or
two-dimensional [
103
] networks (Fig.
17
) are formed depending
on the ability of the tin derivative to function as a mono-, bi-,
or polydentate tecton.
The nitrogen atom of pyridine derivatives forms close
con-tacts with tin along the extensions of not only O–Sn bonds but
also C–Sn, Cl–Sn, Br–Sn, I–Sn, and S–Sn bonds [
99
,
101
,
104
,
105
]. In all cases, the geometric features of the adducts
indicate that the nitrogen lone pair is oriented along the
Fig. 13 Ball and stick representations (Mercury 3.9) of 5-(t-butyl)germatrane (BUWBUQ, left), 5-bromogermatrane (BUWCUR, middle), and phenyl(tris(2-(trimethylsilylamido)ethyl)amine-N,N′,N″)germanium (XUSLOM, right). TBs are depicted as black dotted
lines; hydrogen atoms and methyl substituents on the silyl moieties of XUSLOM have been omitted for clarity. Nc values are shown close to the respective interactions. Color code: gray carbon, red oxygen, light blue nitrogen, bronze bromine, pearl white silicon, light teal germanium
Fig. 14 Ball and stick representations (Mercury 3.9) of 5-methyl-1-aza-5-stannabicyclo(3.3.3)undecane (FEWXOU, left) and 5-fluoro-1-aza-5-stannatricyclo(3.3.3)undecane (ZANKEE, right). TBs are depicted as
black dotted lines; hydrogen atoms have been omitted for clarity. Nc values are shown close to the respective interactions. Color code: gray carbon, light blue nitrogen, yellowish green fluorine, dark teal tin
extension of one of the covalent bonds of tin. For instance, in
the infinite chain formed by the dithiocarbamate reported in
Fig.
18
(refcode UGEFIX), the S
–Sn···N angle is 174.50°, the
geometry around the nitrogen is strictly trigonal planar, and tin
is nearly in the pyridine plane (the two C(sp
2)N···Sn angles are
121.18° and 122.40°, and the distance of tin from the mean
square plane through the pyridine ring is 85 pm).
The cyano group seems to be able to act as an effective TB
acceptor group via the lone pair at the nitrogen. Moreover, due
to its strong electron-withdrawing ability, it is expected that
when the cyano group is directly bound to a tin or germanium
atom, the
σ-hole opposite the covalent NC–Sn/Ge bond will
be particularly positive. Indeed, trimethyltin cyanide (refcode
TIMSNC01) and dimethyltin dicyanide (refcode DMCYSN)
are both self-complementary modules that form infinite chains
[
106
] and square 2D networks [
107
], respectively (Fig.
19
), by
pairing TB donor and TB acceptor sites. Dimethylgermanium
dicyanide (refcode DMCYGE) shows somewhat similar
behavior.
Tetrakis(2-cyanobenzyl)tin (refcode JIWROX) [
108
]
(Fig.
20
) functions as a self-complementary tecton, as the
cyano group of one molecule aligns with the extension of
one of the C
–Sn covalent bonds of an adjacent molecule,
Fig. 15 Ball and stick representations (Mercury 3.9) of (cyclopenta-2,4-dien-1-yl)-(2-(dimethylaminomethyl)phenyl)diphenyltin (left) and (3-aminopropyl)triphenyltin (IHOZAH, right). TBs are depicted as black dotted lines; hydrogen atoms have been omitted for clarity. Nc values are shown close to the respective interactions. Color code: gray carbon, light blue nitrogen, dark teal tin
Fig. 16 Ball and stick
representations (Mercury 3.9) of the trimer formed by (ferrocene-1-carboxylato)triphenyltin and 4,4′-bipyridine (IVUVUR, top) and of the infinite chain formed by
(pyridine-4-carboxylato)tricyclohexyltin (UZAVUN, bottom). TBs are depicted as black dotted lines; hydrogen atoms have been deleted for the sake of simplicity. Nc values are shown close to the respective interactions. Color code: gray carbon, red oxygen, orange iron, light blue nitrogen, dark teal tin
Fig. 17 Ball and stick representation (Mercury 3.9) of the network g e n e r a t e d b y d i ( t r i n b u t y l ) s t a n n y l 5 ( ( p y r i d i n 4 -ylmethylene)amino)isophthalate with 4,4′-bipyridine (TISVEY). TBs are depicted as black dotted lines; three atoms of the butyl residues at tin and hydrogen atoms have been deleted for the sake of simplicity. Nc values are shown close to the respective interactions. Color code: gray carbon, red oxygen, light blue nitrogen, dark teal tin
ultimately forming infinitely long tetrel-bonded ribbons
(Nc = 0.96; the C–Sn···N angle is 178.46°).
In 2-(dimethylaminomethyl)phenyl)cyanodiphenyltin and
bis(2-(dimethylaminomethyl)phenyl)dicyanotin (refcodes
WUVKOP and WUVLOQ, respectively) [
109
], one and two
NC–Sn···N close contacts are present, respectively, and the
amine nitrogen acts as the TB acceptor site in all cases
(Fig.
21
). This may suggest that a N(sp
3) atom is a better TB
acceptor than a N(sp) atom. The same ability to act as a donor
of electron density is observed in XB formation.
Halogen atoms as tetrel bond acceptors
Structures in the CSD reveal that the four halogens F, Cl, Br,
and I can all form close contacts with tetravalent germanium
and tin atoms in organic derivatives. These interactions can be
rationalized as TBs due to the fact that the halogen atom is
located approximately along the extension of one of the
cova-lent bonds formed by the germanium or tin. The bond with the
most electron-withdrawing group is preferentially involved in
the formation of these close contacts.
For instance, crystals of bis(2,5-bis(trifluoromethyl)
phenyl)(dichloro)germane (refcode ZAVCUW) have two
symmetrically nonequivalent molecules in the unit cell
[
110
]. Both of these molecules show two fairly short and
linear TBs oriented along the extensions of the Cl–Ge bonds
(Nc values span the range 0.78–0.79; the C–Ge···F angles are
between 176.15° and 174.93°) (Fig.
22
, left). Analogously, an
values are shown close to the respective interactions. Color code: gray carbon, yellow sulfur, light blue nitrogen, dark teal tin
Fig. 19 Ball and stick representations (Mercury 3.9) of the 1D infinite chain formed by trimethyltin cyanide (TIMSNC01, top) and the 2D network generated by dimethyltin dicyanide (DMCYSN, bottom). TBs are depicted as black dotted lines; hydrogen atoms have been deleted for the sake of simplicity. Nc values are shown close to the respective interactions. Color code: gray carbon, light blue nitrogen, dark teal tin
black dotted lines; hydrogen atoms have been deleted for the sake of simplicity. Nc values are shown close to the respective interactions. Color code: gray carbon, light blue nitrogen, dark teal tin
Fig. 21 Ball and stick representations (Mercury 3.9) of the conformations adopted by cyano-2-(dimethylaminomethyl)phenyl)diphenyltin (WUVKOP, left) and bis(2-(dimethylaminomethyl)phenyl)dicyanotin (WUVLOQ, right). TBs are depicted as black dotted lines; hydrogen atoms have been deleted for the sake of simplicity. Nc values are shown close to the respective interactions. Color code: gray carbon, light blue nitrogen, dark teal tin
intramolecular C
–Ge···F close contact locks in the
conforma-tion of (1,2,3,3,3-pentafluoroprop-1-en-1-yl)triphenyl
ger-manium (refcode ADUKUH) [
111
] in the solid and allows for
the formation of a tetrel-bonded five-membered ring (the Nc
value of Ge···F is 0.86; the C–Ge···F angle is 166.80°). The tin
analog of ADUKUH (refcode ADUKOB) behaves similarly,
as an intramolecular C
–Sn···F TB is present in both of the
independent molecules present in the unit cell of the crystal,
leading to a tetrel-bonded ring (Fig.
22
, right).
Fig. 22 Ball and stick representations (Mercury 3.9) of the conformations adopted by bis(2,5-bis(trifluoromethyl)phenyl)(dichloro)germane (ZAVCUW, left) and (1,2,3,3,3-pentafluoroprop-1-en-1-yl)triphenyltin (ADUKOB, right). TBs are depicted as black dotted lines; hydrogen atoms have been deleted for the sake of simplicity. Nc values are shown close to the respective interactions. Color code: gray carbon, yellowish green fluorine, light teal germanium, dark teal tin
Fig. 23 Ball and stick
representations (Mercury 3.9) of 1D chains generated by fluorotricyclohexyltin (BAJWOY, top),
dichlorodimethyltin (DMSNCL, middle), and dibromodiethyltin (DESNBR, bottom). TBs are depicted as black dotted lines; hydrogen atoms have been omitted for clarity. Nc values are shown close to the respective interactions. Color code: gray carbon, brown bromine, green chlorine, yellowish green fluorine, dark teal tin
Fig. 24 Ball and stick representations (Mercury 3.9) of the conformation adopted by tetrakis(2-chlorobenzyl)tin (CEWGEQ01, left) and the network generated by tetrakis(chloromethyl)tin (UGATEB, right). TBs are depicted as black dotted lines; hydrogen atoms have been omitted for clarity. Nc values are shown close to the respective interactions. Color code: gray carbon, green chlorine, dark teal tin
CEWGEQ) [
117
] provide a nice example of intramolecular
C–Sn···Cl interactions, as three such contacts (Nc values range
from 0.94 to 0.97) lock in the molecular conformation
(Fig.
24
, left). Interestingly, tetrakis(2-methoxybenzyl)tin
(refcode HEVFOD) [
118
] and tetrakis(2-fluorobenzyl)tin
(refcode VULSOM) [
119
] present four intramolecular C–
mine atom is localized along the extension of the Cl–Sn bond
(Nc = 0.78; the Cl–Sn···Br angle is 172.06°) (Fig.
25
, bottom)
[
121
]. Similar Cl–Sn···Br contacts are present in various other
(6-bromo-1,2-dihydroacenaphthylen-5-yl)tin derivatives.
Bromine atoms can also be involved in intermolecular TBs.
Fig. 26 Ball and stick representations (Mercury 3.9) of the conformation adopted by bromo(4-iodo-1,2,3,4-tetraphenyl-1,3-butadienyl)diphenyltin ( S I C S O M , b o t t o m ) a n d t h e n e t w o r k f o r m e d b y tris(trimethylstannyl)ammonium iodide (RONDAZ, top). One layer of RONDAZ is presented, and hydrogen atoms have been omitted for clarity. TBs are depicted as black dotted lines; Nc values are shown close to the respective interactions. Color code: gray carbon, purple iodine, brown bromine, light blue nitrogen, dark teal tin
Fig. 25 Ball and stick representations (Mercury 3.9) of the conformation adopted by chloro(6-bromo-1,2-dihydroacenaphthylen-5-yl)diphenyltin ( V E K K U T, b o t t o m ) a n d t h e 1 D c h a i n g e n e r a t e d b y 3 β-(bromodimethylstannyl)-24-nor-5β-cholane (MISYAO, top). TBs are depicted as black dotted lines; hydrogen atoms have been omitted for clarity. Nc values are shown close to the respective interactions. Color code: gray carbon, brown bromine, dark teal tin
T h i s i s t h e c a s e i n t h e s t e r o i d d e r i v a t i v e
3β-(bromodimethylstannyl)-24-nor-5β-cholane (refcode
MISYAO) [
122
] (Fig.
25
, top), crystals of which include
infi-nitely long 1D chains assembled via Br–Sn···Br.
The covalent bond pathway connecting iodine and tin in
(8-iodo-1-naphthyl)trimethyltin (refcode AQIVUS) [
123
] is
reminiscent of that connecting bromine and tin in VEKKUT,
and this translates into a supramolecular similarity between
the C–Sn···I TB in the former compound and the Cl–Sn···Br
TB in the latter. In the crystal structure of
bromo(4-iodo-1,2,3,4-tetraphenyl-1,3-butadienyl)diphenyltin (refcode
SICSOM) (Fig.
26
, bottom) [
124
], the iodine atom acts as
the TB acceptor and approaches tin—the TB donor—along
the extension of the Br–Sn bond (Nc = 0.94; the Br–Sn···I
angle is 168.95°). This pattern is consistent with the fact that
the most positive
σ-hole on tin is expected to occur at this
position, as bromine is more electron-withdrawing than the
other atoms bound to tin. Finally, the Sn···I interactions
pres-ent in crystals of tris(trimethylstannyl)ammonium iodide
(refcode RONDAZ) [
125
] provide a nice example of
charge-assisted TB. The existence of this type of TB further
high-lights the similarities of the different subsets of
σ-hole
inter-actions, as charge-assisted XBs [
126
] and charge-assisted PBs
[
31
] have already been observed. Specifically, two
crystallo-graphically independent salt units are present in the crystal of
R O N D A Z ; i n b o t h o f t h e s e u n i t s , t h e
tris(trimethylstannyl)ammonium cations act as tridentate TB
donors and the iodide anion as a tridentate TB acceptor, and
3D networks are formed (one 3D network is shown in Fig.
26
,
top).
Conclusions
In this paper, we have reported the results of an analysis of the
CSD that aimed to identify crystal structures of organic
deriv-atives of germanium and tin in which these two elements form
close contacts with lone-pair-possessing atoms.
We focused our attention on close contacts where oxygen,
nitrogen, and halogens were the lone-pair-possessing atoms,
as a wide range of examples of those close contacts were
found in the CSD. However, it may be worth mentioning that
other heteroatoms (e.g., sulfur [
127
–
129
] and phosphorus
[
130
–
132
]) also form similar interactions. Ether and carbonyl
oxygens as well as amine, pyridine, and cyano nitrogens can
all be involved in such interactions, and the geometries
ob-served indicate that the lone pair of the heteroatom is directed
towards the germanium/tin atom independent of the
hybridi-zation of the oxygen/nitrogen atom (which can be sp
3, sp
2, or
sp). Close contacts are formed by derivatives in which
germa-nium and tin atoms bear four carbon residues or where there
are halogen, oxygen, sulfur, or nitrogen substituents instead of
one, two, or three of those carbon residues. Regardless of the
nature and hybridization state of the lone-pair-possessing
at-om, and independent of the nature of the residues that are
covalently bound to germanium and tin, the close contacts
are preferentially formed along the extensions of the covalent
bonds that germanium and tin form with strongly
withdrawing residues. Moreover, the more
electron-withdrawing the residue bound to germanium/tin, the closer
the interaction along the extension of that bond.
All of these features are typical of
σ-hole interactions, so
we propose that the close contacts described in this review
should be termed tetrel bonds. Tetravalent germanium and
tin atoms have a tetrahedral geometry. When these atoms form
one or two close contacts with lone-pair-possessing atoms, the
surrounding geometry tends to change to a trigonal
bipyrami-dal or octahedral geometry, respectively. These changes can
be explained as being due to sp
3→ dsp
3or sp
3→ d
2sp
3rehybridization at the tetrels. They can also be rationalized
by invoking the presence of a tetrel bond [
133
]—an attractive
interaction between a lone pair and a positive
σ-hole along the
extension of a covalent bond formed by the tetrel. The
pres-ence of
σ-holes on all four tetrels is widely supported by
modeling [
38
–
42
], and is also in accord with the
experimen-tally determined geometric features of the interactions
discussed in this review. The rationale for tetrel bonding is
congruent with the other alternative explanations mentioned
above. However, it may offer the additional advantage that
these interactions of group 14 elements can be considered to
be analogous to similar interactions that occur when groups
15–18 elements function as electrophilic sites.
The examined dataset is too limited to be able to draw
general conclusions, but it seems to suggest that the
devi-ation of a tetrel bond from the extension of the relevant
covalent bond to a germanium or tin atom is usually
small-er than the corresponding deviations for most PBs and CBs
[
31
]. This is consistent with theoretical calculations which
show that the region of most positive electrostatic potential
opposite to a covalent bond deviates from the extension of
the bond to the greatest extent in pnictogen derivatives and
to the least extent in tetrel derivatives [
134
,
135
]. The
greater linearity of TBs may be related to the fact that
the electronic asymmetry generated around germanium and
tin atoms by the four residues bonded to them is usually
smaller than the electronic asymmetry generated around
pnictogen and chalcogen atoms by the residues bonded to
them and their lone pair(s) [
136
].
It also seems that steric congestion around the tetrel atoms
studied in this paper plays an influential role in tetrel bond
formation; such steric congestion may even prevent tetrel
bond formation. For instance, tetrakis(2-fluorobenzyl)tin
(refcode VULSOM) forms four intramolecular TBs, whereas
its tetrakis(2-chlorobenzyl) analog (refcode CEWGEQ) forms
t h r e e i n t r a m o l e c u l a r T B s ; a l s o , m e t h y l t r i s ( ( 2
-methoxymethyl)phenyl)germane (refcode IMUTEP) forms
a molecule and/or the network of intermolecular interactions
in the crystal lattice. Tetrel bonds appear to be sufficiently
reliable that they could prove useful tools in crystal
engineering.
Acknowledgements The authors are pleased to recognize the seminal role of Prof. Dr. Peter Politzer in understanding the interactions discussed in this paper as well as sister interactions, all of which are now grouped together under the termBσ-hole bonds.^ The authors are also grateful to Prof. Politzer for fruitful discussions and collaborations regarding this topic.
Open Access This article is distributed under the terms of the Creative C o m m o n s A t t r i b u t i o n 4 . 0 I n t e r n a t i o n a l L i c e n s e ( h t t p : / / creativecommons.org/licenses/by/4.0/), which permits unrestricted use, distribution, and reproduction in any medium, provided you give appro-priate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made.
References
1. Scheiner S (2015) Noncovalent forces. Springer, Cham.https:// doi.org/10.1007/978-3-319-14163-3
2. Kollman PA (1977) Noncovalent interactions. Acc Chem Res 10: 365–371.https://doi.org/10.1021/ar50118a003
3. Riley KE, Pitončák M, Jurecčka P, Hobza P (2010) Stabilization and structure calculations for noncovalent interactions in extended molecular systems based on wave function and density functional theories. Chem Rev 110:5023–5063.https://doi.org/10.1021/ cr1000173
4. Arunan E, Desiraju GR, Klein RA et al (2011) Definition of the hydrogen bond (IUPAC recommendations 2011). Pure Appl Chem 83:1637–1641. https://doi.org/10.1351/PAC-REC-10-01-02
5. Desiraju GR, Steiner T (2001) The weak hydrogen bond in struc-tural chemistry and biology. Oxford University Press, Oxford.
https://doi.org/10.1093/acprof:oso/9780198509707.001.0001
6. Swart M, van der Wijst T, Fonseca Guerra C, Bickelhaupt FM (2007)π–π stacking tackled with density functional theory. J Mol Model 13:1245–1257. https://doi.org/10.1007/s00894-007-0239-y
7. Dougherty DA (2013) The cation–π interaction. Acc Chem Res 46:885–893.https://doi.org/10.1021/ar300265y
8. Schottel BL, Chifotides HT, Dunbar KR (2008) Anion–π interac-tions. Chem Soc Rev 37:68–83.https://doi.org/10.1039/b614208g
9. Jiang XF, Hau FKW, Sun QF, SY Y, Yam VWW (2014) From {AuI···AuI}-coupled cages to the cage-built 2-D {AuI···AuI} ar-rays: AuI···AuIbonding interaction driven self-assembly and their
s00894-008-0386-9
14. Murray JS, Lane P, Clark T, Politzer P (2007)σ-Hole bonding: molecules containing group VI atoms. J Mol Model 13:1033– 1038.https://doi.org/10.1007/s00894-007-0225-4
15. Murray JS, Lane P, Politzer P (2007) A predicted new type of directional noncovalent interaction. Int J Quantum Chem 107: 2286–2292
16. Brinck T, Murray JS, Politzer P (1992) Surface electrostatic po-tentials of halogenated methanes as indicators of directional inter-molecular interactions. Int J Quantum Chem 44:57–64.https://doi. org/10.1002/qua.560440709
17. Brinck T, Murray JS, Politzer P (1993) Molecular surface electro-static potentials and local ionization energies of group V–VII hy-drides and their anions: relationships for aqueous and gas-phase acidities. Int J Quantum Chem 48:73–88.https://doi.org/10.1002/ qua.560480202
18. Politzer P, Murray JS, Clark T (2013) Halogen bonding and other σ-hole interactions: a perspective. Phys Chem Chem Phys 15: 11178–11189.https://doi.org/10.1039/C3CP00054K
19. Wang H, Wang W, Jin WJ (2016)σ-hole bond vs π-hole bond: a comparison based on halogen bond. Chem Rev 116:5072–5104.
https://doi.org/10.1021/acs.chemrev.5b00527
20. Bauzá A, Mooibroek TJ, Frontera A (2015) The bright future of unconventionalσ/π-hole interactions. ChemPhysChem 16:2496– 2517.https://doi.org/10.1002/cphc.201500314
21. Politzer P, Murray JS, Clark T (2013) Halogen bonding and other σ-hole interactions: a perspective. Phys Chem Chem Phys 15: 11178.https://doi.org/10.1039/c3cp00054k
22. Cavallo G, Metrangolo P, Pilati T et al (2014) Naming interactions from the electrophilic site. Cryst Growth Des 14:2697–2702.
https://doi.org/10.1021/cg5001717
23. Terraneo G, Resnati G (2017) Bonding matters. Cryst Growth Des 17:1439–1440.https://doi.org/10.1021/acs.cgd.7b00309
24. Metrangolo P, Pilati T, Resnati G, Stevenazzi A (2003) Halogen bonding driven self-assembly of fluorocarbons and hydrocarbons. Curr Opin Colloid Interface Sci 8:215–222.https://doi.org/10. 1016/S1359-0294(03)00055-4
25. Wang W, Ji B, Zhang Y (2009) Chalcogen bond: a sister noncovalent bond to halogen bond. J Phys Chem A 113:8132– 8135.https://doi.org/10.1021/jp904128b
26. Fick RJ, Kroner GM, Nepal B et al (2016) Sulfur-oxygen chalco-gen bonding mediates AdoMet recognition in the lysine methyl-transferase SET7/9. ACS Chem Biol 11:748–754.https://doi.org/ 10.1021/acschembio.5b00852
27. Nayak SK, Kumar V, Murray JS et al (2017) Fluorination pro-motes chalcogen bonding in crystalline solids. CrystEngComm 19:4955–4959.https://doi.org/10.1039/C7CE01070B
28. Wonner P, Vogel L, Düser M et al (2017) Carbon-halogen bond activation by selenium-based chalcogen bonding. Angew Chem Int Ed 12009–12012.https://doi.org/10.1002/anie.201704816
29. Legon AC (2017) Tetrel, pnictogen and chalcogen bonds identi-fied in the gas phase before they had names: a systematic look at
non-covalent interactions. Phys Chem Chem Phys 19:14884– 14896.https://doi.org/10.1039/C7CP02518A
30. Scheiner S (2013) The pnicogen bond: its relation to hydrogen, halogen, and other noncovalent bonds. Acc Chem Res 46:280– 288.https://doi.org/10.1021/ar3001316
31. Scilabra P, Terraneo G, Resnati G (2017) Fluorinated elements of group 15 as pnictogen bond donor sites. J Fluor Chem 203:62–74.
https://doi.org/10.1016/j.jfluchem.2017.10.002
32. DeBackere JR, Bortolus MR, Schrobilgen GJ (2016) Synthesis and characterization of [XeOXe]2+in the adduct-cation salt,
[CH3CN⋯XeOXe⋯NCCH3][AsF6]2. Angew Chem Int Ed 55:
11917–11920.https://doi.org/10.1002/anie.201606851
33. Grabowski SJ (2014) Tetrel bond-σ-hole bond as a preliminary stage of the SN2 reaction. Phys Chem Chem Phys 16:1824–1834.
https://doi.org/10.1039/c3cp53369g
34. Jonsson B, Karlstrom G, Wennerstrom, H (1975) Ab initio molec-ular orbital calculations on the water–carbon dioxide system: mo-lecular complexes. Chem Phys Lett 30:58–59.https://doi.org/10. 1016/0009-2614(75)85497-2
35. Peterson KI, Klemperer W (1984) Structure and internal rotation of H2O–CO2, HDO–CO2, and D2O–CO2van der Waals
com-plexes. J Chem Phys 80:2439–2445.https://doi.org/10.1063/1. 446993
36. Peng YP, Sharpe SW, Shin SK, Wittig C, Beaudet RA (1992) Infrared spectroscopy of CO2-D(H)Br complex: molecular
struc-ture and its reliability. J Chem Phys 97:5392–5402.https://doi.org/ 10.1063/1.463799
37. Leopold KR, Fraser GT, Klemperer W (1984) Rotational spec-trum and structure of the complex HCN-CO2. J Chem Phys 80:
1039–1046.https://doi.org/10.1063/1.446830
38. Mani D, Arunan E (2013) The X–C⋯Y (X = O/F, Y = O/S/F/Cl/ Br/N/P)Bcarbon bond^ and hydrophobic interactions. Phys Chem Chem Phys 15:14377–14383.https://doi.org/10.1039/c3cp51658j
39. Bauzá A, Mooibroek TJ, Frontera A (2013) Tetrel-bonding inter-action: rediscovered supramolecular force? Angew Chem Int Ed 52:12317–12321.https://doi.org/10.1002/anie.201306501
40. Liu M, Li Q, Scheiner S (2017) Comparison of tetrel bonds in neutral and protonated complexes of pyridineTF3and furanTF3(T
= C, Si, and Ge) with NH3. Phys Chem Chem Phys 19:5550–
5559.https://doi.org/10.1039/C6CP07531B
41. Alkorta I, Rozas I, Elguero J (2001) Molecular complexes be-tween silicon derivatives and electron-rich groups. J Phys Chem A 105: 743–749.https://doi.org/10.1021/jp002808b
42. Grabowski SJ (2017) Lewis acid properties of tetrel tetrafluo-rides—the coincidence of the σ-hole concept with the QTAIM approach. Crystals 7:43.https://doi.org/10.3390/cryst7020043
43. Southern SA, Bryce DL (2015) NMR investigations of noncovalent carbon tetrel bonds. Computational assessment and initial experimental observation. J Phys Chem A 119:11891– 11899.https://doi.org/10.1021/acs.jpca.5b10848
44. Mahmoudi G, Bauzá A, Frontera A (2016) Concurrent agostic and tetrel bonding interactions in lead(II) complexes with an isonicotinohydrazide based ligand and several anions. Dalton Trans 45:4965–4969.https://doi.org/10.1039/c6dt00131a
45. Cheng F, Hector AL, Levason W et al (2009) Preparation and structure of the unique silicon(IV) cation [SiF3(Me3tacn)]+.
Chem Commun 1334–1336.https://doi.org/10.1039/b822236c
46. Bondi A (1964) Van der Waals volumes and radii. J Phys Chem 68:441–451.https://doi.org/10.1021/j100785a001
47. Batsanov SS (2001) Van der Waals radii of elements. Inorg Mater 37:871–885.https://doi.org/10.1023/A:1011625728803
48. Jambor R, Dostál L, Růžička A, Císařová I, Brus J, Holčapek M, Holeček J (2002) Organotin(IV) derivatives of some O,C,O-che-lating ligands. Organometallics 21:3996–4004.https://doi.org/10. 1021/om020361i
49. Dostál L, Jambor R, Růžička A et al (2007) Organotin(IV) deriv-atives of some O,C,O-chelating ligands. Part 2. Organometallics 26:6312–6319.https://doi.org/10.1021/om700576n
50. Scheiner S (2017) Systematic elucidation of factors that influence the strength of tetrel bonds. J Phys Chem A 121:5561–5568.
https://doi.org/10.1021/acs.jpca.7b05300
51. Sugiyama Y, Matsumoto T, Yamamoto H et al (2003) Synthesis, s o l i d s t a t e a n d s o l u t i o n s t r u c t u r e s o f t r i s [ ( 2 -methoxymethyl)phenyl]germanes with a substituent on germani-um. Tetrahedron 59:8689–8696.https://doi.org/10.1016/j.tet. 2003.09.053
52. Shindo M, Matsumoto K, Shishido K (2007) Hyperconjugative effect of C-Ge bonds: synthesis of multisubstituted alkenylgermanes via torquoselective olefination of acylgermanes with ynolates. Tetrahedron 63:4271–4277.https://doi.org/10. 1016/j.tet.2007.03.048
53. Jousseaume B, Villeneuve PM, Driiger Roller S, Chezeau JM ( 1 9 8 8 ) U n i q u e t i n–oxygen coordination bond in a pentacoordinated tetraorganotin compound. First confirmation b y X r a y c r y s t a l s t r u c t u r e o f ( 2 c a r b o m e t h o xy 1 , 4 -cyclohexadien-1-yl) trimethyltin. J Organomet Chem 349:C1– C3.https://doi.org/10.1016/0022-328X(88)80459-5
54. Beak P, Lee WK (1993)α-Lithioamine synthetic equivalents: syntheses of diastereoisomers from Boc derivatives of cyclic amines. J Org Chem 58:1109–1117.https://doi.org/10.1021/ jo00057a024
55. Cintrat JC, Léat-Crest V, Parrain JL, et al (2004) Identification of chiral cis- and trans-2-stannyloxazolidines by their NMR spectra and solid-state structures. Eur J Org Chem 4268–4279.https://doi. org/10.1002/ejoc.200400203
56. Gurkova SN, Gusev AI, Alekseev NV, Gar TK, Viktorov NA (1984) Intramolecular interactions in germanium compounds. Crystal and molecular structures of the N,N′-dimethylamide of 2-methyl-3-(trichlorogermyl) propionic acid and 1-(1-trichlorogermyl) pyrrolid-2-one. J Struct Chem 25:825–828 57. Deka DC, Helliwell M, Thomas EJ (2001) Synthesis of chiral
organotin reagents: synthesis and X-ray crystal structures of bicyclo[2.2.1]heptan-2-yl(diphenyl)tin chlorides with cis-dis-posed nitrogen containing substituents. Tetrahedron 57:10017– 10026.https://doi.org/10.1016/S0040-4020(01)01035-3
58. Tretyakov EV, Mareev AV, Demina MM et al (2009) Silyl- and germylpropynals in the synthesis of azolyl-substituted 2-imidazoline 3-oxide 1-oxyls. Russ Chem Bull. 58:1915–1920.
https://doi.org/10.1007/s11172-009-0261-6
59. Gurkova SN, Gusev AI, Alekseev NV, Gar TK, Viktorov NA (1984) Intramolecular interactions in germanium compounds. Crystal and molecular structure of 1,3-diphenyl-3-methyl-3-(trichlorogermyl)-butan-1-one. J Struct Chem 25:829–831 60. Wang LB (2007) (μ-2,2′-Biquinolinyl-4,4′-dicarboxylato-κ2O :
O′)bis[(dimethylformamide-κ O)triphenyltin(IV)]. Acta Crystallogr E 63:m1883–m1883. https://doi.org/10.1107/ S1600536807028048
61. Lorberth J, Shin S, Donath H, Wacadlo S, Massa W (1991) Metalorganic diazoalkanes: XX. Crystal structure of trimethyltin diazoacetic ester, Me3SnC(N2CO2Et. J Organomet Chem 407:
167–171
62. Lukevics E, Arsenyan P, Belyakov S et al (1999) Cycloaddition reactions of nitrile oxides to silyl- and germyl-substituted thio-phene-1,1-dioxides. Organometallics 18:3187–3193.https://doi. org/10.1021/om9902129
63. Chuprunov EV, Stolyarova NE, Shcherbakov VI, Tarkhova TN (1988) Crystal structure of N-triethylstannylsuccinimide. J Struct Chem 28:797–799
64. Jaray O, Pritzkow H, Jander J (1977) X-ray structural analysis of organic N-Br compounds for making visible general structure el-ements of bromamines. Z Naturforsch 32b:1416–1420
68. Uehara K, Nakao H, Kawamoto R et al (2006) 2D-grid layered pd-based cationic infinite coordination polymer/polyoxometalate crystal with hydrophilic sorption. Inorg Chem 45:9448–9453.
https://doi.org/10.1021/ic061393r
6 9 . Ta y l o r P, P o l l E , O l b r i c h F, F i s c h e r R D ( 2 0 1 4 ) [Sn2(H2O)2Br2(CH3)4{μ-(CH2)3}·2bpy]: a layered, hetero
bimo-lecular composite (bpy=2,2-bipyridine). Supramol Chem 10: 2014.https://doi.org/10.1080/10610270290029344
70. Reeske G, Schürmann M, Costisella B, Jurkschat K (2005) Organotin-substituted crown ethers for ditopic complexation of anions and cations. Eur J Inorg Chem 2881–2887.https://doi. org/10.1002/ejic.200500191
71. Mandolesi S, Studentkowski M, Preut H, Mitchell T (2001) A 1:1 adduct between 2,2-bis(chlorodimethylstannyl)propane and di-methyl sulfoxide. Acta Crystallogr E 57:m543–m544.https:// doi.org/10.1107/S1600536801017603
72. Zhu FC, Shao PX, Yao XK et al (1990) Stereochemistry and crystal structures of triphenyltin chloride complexes with bis(phenylsulfinyl)ethane. Inorg Chim Acta 171:85–88.https:// doi.org/10.1016/S0020-1693(00)84669-1
73. Kumar S, Shadab SM, Idrees M (2009) Chlorido(dimethyl sulf-oxide-κO)triphenyltin(IV). Acta Crystallogr E 65:m1602–m1603.
https://doi.org/10.1107/S1600536809048090
7 4 . H o w i e R A , W a r d e l l J L ( 1 9 9 4 ) S t r u c t u r e s o f P h3S n C H2C H2C H2S O2C6H4M e - p a n d
IPh2SnCH2CH2CH2SO2C6H4Me-p. Main Group Met Chem.
17:571–582.https://doi.org/10.1515/MGMC.1994.17.8.571
75. Lo KM, Ng SW (2011) Tribenzyl-chlorido(triphenyl-phosphine oxide-κO)tin(IV). Acta Crystallogr E 67:112–122.https://doi. org/10.1107/S160053681101957X
76. Lo KM, Ng SW (2004) [Chlorobis(p -chlorophenyl)(p-tolyl)tin]-μ-1,2-bis(diphenylphosphoryl)ethane-κ2
O:O ′-[bromobis(p-chlorophenyl)(p-tolyl)tin]. Acta Crystallogr E 60:m717–m719.
https://doi.org/10.1107/S1600536804010219
7 7 . P r e u t H , G o d r y B , M i t c h e l l T N ( 1 9 9 2 ) [ 2 -(Bromodimethylstannyl)ethyl]diphenylphosphine sulfide. Acta Crystallogr Sect C 48:1491–1493.https://doi.org/10.1107/ S0108270191014750
78. Shariatinia Z, Mirhosseini Mousavi HS, Bereciartua PJ, Dusek M (2013) Structures of a novel phosphoric triamide and its organotin(IV) complex. J Organomet Chem 745–746:432–438.
https://doi.org/10.1016/j.jorganchem.2013.08.003
79. Jurkschat K, Tzschach A, Meunierpiret J (1986) Synthesis, crystal a n d m o l e c u l a r s t r u c t u r e o f 1 A Z A 5 S TA N N A 5 -methyltricyclo[3.3.3.01,5]undecane. Evidence for a transannular donor–acceptor interaction in a tetraorganotin compound. J Organomet Chem 315:45–49. https://doi.org/10.1016/0022-328X(86)80409-0
80. Jurkschat K, Hesselbarth F, Dargatz M, Lehmann J, Kleinpeter E, Tzschach A, Meunierpiret J (1990) 1,2-Bis(organostannyl)ethanes as powerful bidentate Lewis acids. Crystal structures of ( P h2C l S n C H 2)2· · · ( M e 2N )2P O a n d
Organometallics 20:2730–2735.https://doi.org/10.1021/ om0009738
84. Gurkova SN, Gusev AI, Alekseev NV, Segel’man RI, Gar TK, Khromova NY (1983) Crystal and molecular structure of 1-(tert-butyl)germatrane. J Struct Chem 24:155–157.https://doi.org/10. 1021/ic50138a020
85. Gurkova SN, Gusev AI, Alekseev NV, Segel’man RI, Gar TK, Khromova NYu (1983) Crystal and molecular structure of 1-bromogermatrane. J Struct Chem 24:238–241.https://doi.org/10. 1007/BF00747386
86. Gurkova SN, Gusev AI, Alekseev NV, Segel’man RI, Gar TK, Khromova NY (1981) Crystal and molecular structure of Iodomethylgermatrane. J Struct Chem 22:461–462
87. Gurkova SN, Gusev AI, Alekseev NV, Gar TK, Khromova NY (1981) Crystal and molecular structure of 1-methyl-2-carbagermatrane. J Struct Chem 22:924–926
88. Gurkova SN, Gusev AI, Alekseev NV, Gar TK, Viktorov NA (1985) Crystal and molecular structure of 1-(germatranyl)-1-(2-pyrrolidonyl)ethane. J Struct Chem 26:124–127
89. Shutov PL, Sorokin DA, Karlov SS et al (2003) Azametallatranes of group 14 elements. Syntheses and X-ray studies. Organometallics 22:516–522. https://doi.org/10.1021/ om020708h
90. Karlov SS, Lermontova EK, Zabalov MV et al (2005) Synthesis, X - r a y d i ff r a c t i o n s t u di e s, a nd D F T c a l c u l a t i o ns o n hexacoordinated germanium derivatives: the case of germaspirobis(ocanes). Inorg Chem 44:4879–4886.https://doi. org/10.1021/ic048165m
91. Jurkschat K, Kolb U, Dräger M, Dargatz M (1995) Unusual hexacoordination in a triorganotin fluoride supported by intermo-lecular hydrogen bonds. Crystal and mointermo-lecular structures of 1-aza-5 - s t a n n a - 1-aza-5 - h a l o g e n o t r i c y c l o [ 3 . 3 . 3 . 0 1 . 1-aza-5 ] u n d e c a n e s N(CH2CH2CH2)3SnF·H2O and N(CH2CH2CH2)3SnX (X = Cl,
Br, I). Organometallics 14:2827–2834.https://doi.org/10.1021/ om00006a031
92. Jurkschat K, Tzschach A (1985) Crystal and molecular structure of 1-aza-5-stanna-5-chlorotricyclo[3.3.3]undecane, a 2,8,9-tricarbastannatrane. J Organomet Chem 290:285–289
93. Turek J, Padělková Z, Černošek Z et al (2009) C,N-chelated hexaorganodistannanes, and triorganotin(IV) hydrides and cyclopentadienides. J Organomet Chem 694:3000–3007.https:// doi.org/10.1016/j.jorganchem.2009.04.043
94. Růžička A, Padělková Z, Švec P et al (2013) Quest for triorganotin(IV) compounds containing three C,N- and N,C,N-chelating ligands. J Organomet Chem 732:47–57.https://doi. org/10.1016/j.jorganchem.2013.02.018
95. Kawachi A, Tanaka Y, Tamao K (1999) Synthesis and structures of a series of Ge-M (M=C, Si, and Sn) compounds derived from germyllithium containing three 2-(dimethylamino)phenyl groups on germanium. J Organomet Chem 590:15–24.https://doi.org/10. 1016/S0022-328X(99)00386-1
96. Novák P, Císařová I, Jambor R et al (2004) Coordination behav-iour of the 2-(N,N-dimethylaminomethyl)phenyl ligand towards